I got part A to this question but I need part B and C!!! Thank you! A buffer is

Question

I got part A to this question but I need part B and C!!! Thank you!

A buffer is prepared by adding 10.0 g of ammonium chloride (NH4Cl) to 250 mL of 1.00 MNH3 solution.

Part A: What is the pH of this buffer? The answer is 9.38.

Part B: Write the net ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer.

Express your answer as a chemical equation. Identify all of the phases in your answer.

Part C: Write the net ionic equation for the reaction that occurs when a few drops of potassium hydroxide solution are added to the buffer.

Express your answer as a chemical equation. Identify all of the phases in your answer.

Explanation / Answer

when we add Nitric acid net ionic equation will be

H+ (aq) + NO3- (aq) + NH3 (aq) --------> NH4+ (aq) + NO3- (aq)

when we add KOH net ionic equation will be

K+ (aq) + OH- +  NH4+ (aq) + Cl- (aq) --------> K+ (aq) + NH3 (aq) + H2O (l) + Cl- (aq)

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